[tex]
\begin{array}{|l|l|}
\hline
\text{Ideal gas law} & P V = n R T \\
\hline
\text{Ideal gas constant} & R = 8.314 \left[ \frac{L \cdot kPa}{mol \cdot K} \right] \\
\hline
\text{Celsius to Kelvin conversion} & 1 \, \text{atm} = 101.3 \, \text{kPa} \\
\hline
\end{array}
[/tex]

The gas in a sealed container has an absolute pressure of 125.4 kilopascals. If the air around the container is at a pressure of 99.8 kilopascals, what is the gauge pressure inside the container?

A. [tex]1.5 \, \text{kPa}[/tex]
B. [tex]24.1 \, \text{kPa}[/tex]
C. [tex]25.6 \, \text{kPa}[/tex]
D. [tex]112.6 \, \text{kPa}[/tex]
E. [tex]225.2 \, \text{kPa}[/tex]

To find the gauge pressure inside the container, we need to understand the difference between absolute pressure and gauge pressure:

1. Absolute Pressure is the total pressure inside the container. It's the pressure reading that includes the atmospheric pressure outside the container.

2. Gauge Pressure is the difference between the absolute pressure inside the container and the atmospheric pressure outside the container. It doesn't take atmospheric pressure into account and is the pressure that a gauge would read.

Here's how to calculate the gauge pressure:

- Step 1: Identify the absolute pressure inside the container. According to the details given, this is 125.4 kilopascals (kPa).

- Step 2: Identify the atmospheric pressure outside the container. The problem states this is 99.8 kPa.

- Step 3: Calculate the gauge pressure by subtracting the atmospheric pressure from the absolute pressure:

[tex]\[
\text{Gauge Pressure} = \text{Absolute Pressure} - \text{Atmospheric Pressure}
\][/tex]

[tex]\[
\text{Gauge Pressure} = 125.4 \, \text{kPa} - 99.8 \, \text{kPa} = 25.6 \, \text{kPa}
\][/tex]

Therefore, the gauge pressure inside the container is 25.6 kPa. Hence, the correct answer is:

C. [tex]\( 25.6 \, \text{kPa} \)[/tex]